Chemistry - Unit 3: Electronic Structure

metals

left of the staircase

usually solid

high melting point

shiny

malleable

good conductor

ready to lose electrons

nonmetals

right of the staircase

usually gas

low melting point

dull

brittle

poor conductor

ready to gain electrons

metalloids

on the staircase

moderate melting point

shiny or dull

malleable

medium conductor

lose/gains electrons

alkali metals

alkaline earth metals

transition metals

inner transition metals

halogens

noble gases

metalloids

other metals

other non-metals

atomic size _____ as you move down a group

increases

atomic size ______ as you move across a period

decreases

ionization energy _____ as you move down a group

decreases

ionization energy ______ as you move across a period

increases

electronegativity ______ as you move down a group

decreases

electronegativity _____ as you move across a period

increases

alkali metals

1 valance e-

very high reactivity

soft metals

group 1

alkaline earth metals

2 valence e-

high reactivity

soft metals (harder than group 1)

group 2

transition metals

valence e- varies

moderate reactivity

hard metals

good heat/electrical conductors

groups 3-12(d block)

inner transition metals

valence e- varies

moderate reactivity

behave like alkali metals

all radioactive

halogens

7 valence e-

moderate reactivity

often form salts with metals

group 17

noble gas

8 valence e-

low-hone reactivity

mendeleev

arranged elements in order of increasing atomic mass

moseley

realized elements should be arranged by increasing atomic number

energy level

distance of the orbital from the nucleus

aufbau principle

states an electron will occupy the lowest energy orbital

schrodinger

determined the probability of finding an electron in various locations around the nucleus

electronegativity

ability to attract electrons when it a part of a compound

ionization

amount of energy required to remove e- from an atom